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Chemical Bonds: Simplified surface view of a molecule.
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<font face="Verdana, Arial, Helvetica, sans-serif" size="5" color="#FFFFFF"><strong>Chemical Bonds:</strong> Simplified surface view of a molecule.</font>
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<td><img src="atomMainIdea.png" width="98" height="58"></td>
<td><font face="Verdana, Arial, Helvetica, sans-serif" size="4">The three major categories of bond types are: non-polar covalent, polar covalent, and ionic. Electronegativity or the ability for an atom to attract another atom's electrons is the key. Below is an introduction to one way of visualizing the way electrons are shared (or not) between atoms.</font></td>
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<font size="4" face="Verdana, Arial, Helvetica, sans-serif">This is
a view of the simplest two atom molecule. In the next few pages you
will explore the types of bonds that can form between two atoms. To
facilitate your understanding, a simplified view of the electrons
will be shown. </font>
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<img width="343" src="surfaceDiagramComp.png" height="123">
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<img width="209" src="surfaceChargeComp.png" height="332">
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<font size="4" face="Verdana, Arial, Helvetica, sans-serif">The
three main categories of bonds (non-polar covalent, polar covalent,
and ionic) are formed when electrons are shared in varying degrees
between atoms. The sharing can be as follows:</font>
<ul>
<li>
<font size="4" face="Verdana, Arial, Helvetica, sans-serif">completely
equal or only slightly unequal sharing </font>
</li>
<li>
<font size="4" face="Verdana, Arial, Helvetica, sans-serif">somewhat
unequal sharing </font>
</li>
<li>
<font size="4" face="Verdana, Arial, Helvetica, sans-serif">so
imbalanced that we don't really consider the electrons to be
shared, but instead they are thought of as transferred from one
atom to another</font>
</li>
</ul>
<p>
<font size="4" face="Verdana, Arial, Helvetica, sans-serif">When
electrons are shared evenly, the entire surface of the molecule
shows no imbalance of charge. However, when electrons tend to be
found closer to one atom versus another, the surface of the
molecule near the atom with the better hold on the electrons
becomes relatively more negative than the surface near the other
atom (which becomes relatively positive). </font>
</p>
<p>
<strong><font size="4" face="Verdana, Arial, Helvetica, sans-serif">Electronegativity
is the term used to describe how well an atom attracts electrons
from another atom.</font></strong><font size="4" face="Verdana, Arial, Helvetica, sans-serif">
</font>
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<font size="4" color="#000000" face="Verdana, Arial, Helvetica, sans-serif">The
picture of a molecule that is colored slightly red and blue shows a bond
between two atoms. One atom has a higher electronegativity than the other.</font><font size="4" color="#660000" face="Verdana, Arial, Helvetica, sans-serif">
<strong>Right-click (or control click) on the red-white-and-blue molecule,
select "annotate" from the popup menu, and use the annotation tools ( <img height="15" width="16" src="textAnnotation.gif">
 <img height="14" width="15" src="drawLine.gif">  <img height="12" width="16" src="drawRect.gif">
) at the top of the new window to label which atom has the higher
electronegativity. Explain your choice in the text area below the picture.</strong></font>
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